The gas—liquid coexistence curve is shown by the blue line, terminating at the critical point the solid blue circle. The dashed lines demarcates the regions where N2 is neither a supercritical fluid, a liquid, nor a gas. This coefficient may be either positive corresponding to cooling or negative heating ; the regions where each occurs for molecular nitrogen, N2, are shown in the figure. Note that most conditions in the figure correspond to N2 being a supercritical fluid , where it has some properties of a gas and some of a liquid, but can not be really described as being either.
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The gas—liquid coexistence curve is shown by the blue line, terminating at the critical point the solid blue circle. The dashed lines demarcates the regions where N2 is neither a supercritical fluid, a liquid, nor a gas. This coefficient may be either positive corresponding to cooling or negative heating ; the regions where each occurs for molecular nitrogen, N2, are shown in the figure.
Note that most conditions in the figure correspond to N2 being a supercritical fluid , where it has some properties of a gas and some of a liquid, but can not be really described as being either. The coefficient is negative at both very high and very low temperatures; at very high pressure it is negative at all temperatures.
The maximum inversion temperature K for N2 [10] occurs as zero pressure is approached. At temperatures below the gas-liquid coexistence curve , N2 condenses to form a liquid and the coefficient again becomes negative. Thus, for N2 gas below K, a Joule—Thomson expansion can be used to cool the gas until liquid N2 forms.
Physical mechanism[ edit ] There are two factors that can change the temperature of a fluid during an adiabatic expansion: a change in internal energy or the conversion between potential and kinetic internal energy.
Temperature is the measure of thermal kinetic energy energy associated with molecular motion ; so a change in temperature indicates a change in thermal kinetic energy. The internal energy is the sum of thermal kinetic energy and thermal potential energy.
This is what happens in a Joule—Thomson expansion and can produce larger heating or cooling than observed in a free expansion. In a Joule—Thomson expansion the enthalpy remains constant. The enthalpy, H.
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